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Question

Given below are the half-cell reactions:
Mn2++2eMn;Eo=1.18V
2(Mn3++eMn2+);Eo=+1.51V
The Eo for 3Mn2+Mn+2Mn3+ will be:
  1. 0.33V; the reaction will occur
  2. 2.69V; the reaction will not occur
  3. 2.69V; the reaction will occur
  4. 0.33V; the reaction will not occur

A
0.33V; the reaction will not occur
B
0.33V; the reaction will occur
C
2.69V; the reaction will not occur
D
2.69V; the reaction will occur
Solution
Verified by Toppr

The correct option is C 2.69V; the reaction will not occur
Standard electrode potential of reaction will not change due to multiply the half-cell reactions with some numbers,
To get the main eq we have to reverse 2nd equation and add them
So E3=E2+E1
E3=1.18+(1.51)
E3=2.69V
The reaction is not possible as the ΔG will come +ve for this case and that indicates reaction is non-spontaneous.

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Similar Questions
Q1
Given below are the half-cell reactions:
Mn2++2eMn;Eo=1.18V
2(Mn3++eMn2+);Eo=+1.51V
The Eo for 3Mn2+Mn+2Mn3+ will be:
View Solution
Q2
Given below are the half-cell reactions
Mn2++2eMn,Eo=1.18V
2(Mn3++eMn2+),Eo=+1.51V
The Eo for 3Mn2+Mn+2Mn3+ will be:
View Solution
Q3

Given below are the half-cell reaction:
Mn2++2eMn; E=1.18V
2(Mn3++eMn2+; E=+1.51V

The E for 3Mn2+Mn+2Mn3+ will be:
(IIT-JEE 2014)


View Solution
Q4
Given below are the half-cell reaction:
Mn2++2eMn; E=1.18V
2(Mn3++eMn2+; E=+1.51V

The E for 3Mn2+Mn+2Mn3+ will be:
(IIT-JEE 2014)
View Solution
Q5
Given below are the half-cell reactions:
Mn2++2eMn; E=1.18V
2(Mn3++eMn2+); E=+1.51 V
The E for 3Mn2+Mn+2Mn3+ will be:

View Solution